Download Atoms of an element are identical

1. State the main ideas of Dalton’s Atomic Theory.
2. What experiments and theories regarding the atom came prior to
Dalton? Explain these theories.
a.
b.
c.
d.
Thomson
Milliken
Rutherford
Chadwick
3. What did Rutherford’s gold foil experiment tell us about the structure of the
atom?
4. Draw the Bohr Model of the atom for sodium.
5. Describe the composition of the nucleus of the atom.
6. What does the atomic number of each atom represent? Who is credited
with the study of atomic numbers?
7. Distinguish between mass number and atomic number.
8. List the subatomic particles with charge, location, and approximate mass.
9. What is an amu?
10. How does the modern quantum mechanical atomic model differ from the
atom of Dalton?
11. Why is there an average atomic mass on the periodic table?
12. Complete the following table.
Nuclid Element
#
Mass
e
Proto #
ns
Hydrogen
C-14
Carbon
14
19
#
Electron
s
Atomic
Number
#
Isotope,
Neutrons Ion, or
Neutral
17
37
Calcium
4
5
Uranium
Neutral
235
10
12
13. Referring to the reference table for the Bohr model for the following
questions
a. For n = 1 an electron is at its ground state if it jumps up to level 4,
what state is it?
b. If the same electron drops back to its ground state, the light energy
emitted is in which general region of the Electromagnetic spectrum
c. Where is visible light located in the region of the electromagnetic
spectrum in meters?
3. Dalton’s atomic theory and the Law of Multiple Proportions holds
true with some major exceptions
a. change mass to _______ _______ ________
b. subatomic particles found were_________, _________, _______
4. Subatomic Particles:
In the middle of the 19th century further experimentation led to the discovery
of the ___________, ____________, and ________
Rays move from the ___________ to the ___________, therefore these
rays were named ___________ rays and were composed of
_____________.
p.76 JJ Thomson discovered the _____________ and determined it’s
charge to mass ratio. In addition, JJ Thomson discovered another
subatomic particle, the ________.
p.77_____________determined the first accurate measurement of an
electron’s charge (-1) in his famous ________ __________experiment.
Different drops had different charges but were all found to be multiples of
one small _____.
________ ___________ predicted the presence of the neutron, however
_____________ discovered the neutron.
p. 80 Atoms of the same element that differ in mass are _________.
Using X-rays, ___________found that the wavelength of the X-rays were
characteristic of the particular metal being tested. He determined the
______ ______ of the element which is represented by the letter ____ p.
83.
The number of ______ determines the identity of an element and the
number of ____ determines the particular isotope of the elemtent.
A particular kind of atom containing a definite number of protons and
neutrons is called a ______. p.84 Any isotope of any element is called
_______.
The number of neutrons = _______ - _________
______________ gold foil experiment determined that the nucleus is very
very _______ and that most of the atom is occupied by __________ space
p.78.
p.809
___________ are rays that are spontaneously emitted from unstable atomic
nuclei. These rays can be particles or energy. This is no ordinary chemical
reaction. __________ theorized that mass and energy are equivalent in the
following equation ______= _________
(Energy is in ________, mass is in _______ and the speed of light is in
____________)
Since the nucleus is composed of protons and neutrons, nuclear forces hold
the nucleus together and are very powerful in order to overcome the
repulsive forces of all the positive charges.
Radiation p. 809
________ particle is a helium nucleus composed of two _______ and two
_________. A _______particle is a high speed __________ emitted from a
radioactive ________. _________ _________ are very high energy X
rays.
Dalton’s Atomic Theory
Dalton
Today
Matter is composed of very tiny or
microscopic particles called
“Atom”.
Atom is an indivisible particle
Atom can never be created nor it
is destroyed.
Atoms of an element are identical
in size, shape, mass, and in other
properties.
Atoms of different elements are
different in their properties.
Atoms combine with each other in
small whole numbers.
_____1. Which of the following is NOT part of Dalton’s model of the atom?
a. The atom is unchanged in chemical reactions.
b. The atom is
invisible.
c. The atom has most of its mass in the center.
d. The atom is
indivisible.
_____2. Which of the following statements was NOT part of Dalton’s hypothesis
on the structure of matter?
a. All matter is made up of atoms.
b. Atoms of the same element are identical.
c. Atoms are made of protons and electrons
d. Atoms unite in definite ratios to form compounds.
_____3. According to the law definite proportions, any two samples of potassium
chloride have
a. The same mass.
b. Slightly different molecular
structures.
c. The same melting point.
d. The same ratio of elements.
_____4. According to the law of conservation of mass, when sodium, hydrogen,
and oxygen react to form a
compound, the mass of the compound is _________ the sum of the
masses of the individual elements.
a. Equal to.
b. Greater than.
c. Less than.
d. Either greater
than or less than.
_____5. According to Dalton’s atomic theory, atoms
a. Are destroyed in chemical reaction
b. Can be divided
c. Of each element are identical in size, mass, and other properties
d. Of different elements cannot combine
_____6. Which of the following is NOT part of Dalton’s atomic theory?
a. Atoms cannot be divided, created, or destroyed
b. The number of protons in an atom is its atomic number
c. In a chemical reaction atoms are combined.
d. All matter is composed of extremely small particles called atoms
_____7. According to Dalton’s atomic theory, atoms
a. Of different elements combine in simple whole-number ratios to form
compounds
b. Can be divided into protons, neutrons, and electrons
c. Of all elements are identical in size and mass
d. Can be destroyed in chemical reactions
_____8. Dalton’s theory essentially agreed with the present atomic theory
EXCEPT for the statement that
a. All matter is made up of small particles called atoms
b. Atoms are not divided in chemical reaction
c. Atoms of the same element are chemically alike
d. All atoms of the same element have the same mass
_____9. Which concept in Dalton’s atomic theory has been modified?
a. All matter is composed of atoms
b. Atoms of different elements have different properties and masses
c. Atoms can combine in chemical reaction
d. Atoms cannot be divided
_____10. When electrical current passed through a glass tube, a paddle wheel
placed between the anode and the cathode
moved. Scientists concluded that
a. A magnetic field was produced b. Particles were passing from the
cathode to the anode
c. There was gas in the tube
d. Atom were indivisible
_____11. The ray produced in a cathode tube in early experiment were
a. Unaffected by a magnetic field b. Deflected away from a negative plate
c. Found to carry a positive charge
d. Striking the cathode
_____12. The behavior of cathode rays produced in a glass tube containing gas
at low pressure led scientists to conclude
that the rays
a. Were not composed of matter
b. Were composed
of positively charged particles
c. Were composed of negatively charged particles
d. Were composed
of uncharged particles
_____13. Experiments with cathode rays led to discovery of the
a. Proton
b. Nucleus c. Neutrons d. Electron
_____14. Millikan’s experiments
a. Demonstrated that the electron carried no charged
b. Demonstrated that the electron carried the smallest possible positive
charge
c. Measured the charge on the electron
d. Atoms carried a negative charged
_____15. By analyzing the data from hundreds of experiments, Millikan found
that oil droplets carried an electric charge
a. that was not related to other oil droplets.
b. that was attracted to
the negatively charge plate.
c. that was equal to a fundamental unit of charge. d. that caused it to be
attracted to other oil droplets.
_____16. In Rutherford’s experiment very few positively charged alpha particles
a. Were slightly deflected as they passed through the metal b. Were used
to bombard a cathode plate
c. Collided with electrons
d. Were used to
bombard thin metal foil
_____17. In Rutherford’s experiment, most of the particles
a. Bounced back
b. Passed through the foil
c. Were absorbed by the foil
d. Combined with the foil
_____18. Because most particles fired at metal foil passed straight through,
Rutherford concluded that
a. Atoms were mostly empty space
b. Atoms contained no
charged particles
c. Electron formed the nucleus
d. Atoms were indivisible
_____19. Because a few positively charged particles bounced back from the foil,
Rutherford concluded that such particles
were
a. Striking electrons b. Indivisible c. Repelled by dense regions of positive
charge d. Magnetic
_____20. Rutherford’s experiment led to the discovery of the
a. Electron b. Cathode ray
c. Nucleus
d. Neutron
_____21. Rutherford’s experimental results led him to conclude that atoms
contain massive central regions that have
a. A positive charge
b. A negative charge
c. No charge
d. Both protons and electrons
_____22. Rutherford’s fired positively charged particles at metal foil and
concluded that most of the mass of an atom was
a. In the electrons
b. Concentrated in the nucleus
c. Evenly spread throughout the atom
d. In rings around the atom
_____23. The Greek philosopher that first proposed the idea of atoms was
a. Aristotle b. Dalton c. Plato d. Democritus
_____24. The Greek philosopher that first came up with the Four Element
Theory of Matter was
a. Aristotle b. Dalton c. Plato d. Democritus